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Oxidation reaction involves loss of elec...

Oxidation reaction involves loss of electrons, and reduction reaction involves gain of electrons. The reaction in which a species disproportinates into two oxidation states ( lower and higher) is called disproportionation reaction.
Which of the following statements is wrong?

A

The algebraic sum of the oxidation numbers of all atoms in an ion is zero.

B

The oxidation number is an arbitrary number. It can have positive, negative, zero, or fractional values.

C

When a negative ion changes to neutral species, the process is oxidation.

D

The oxidation number of phosphorous can very from `-3 t o +5`.

Text Solution

AI Generated Solution

The correct Answer is:
To determine which statement is wrong regarding oxidation, reduction, and disproportionation reactions, we will analyze each statement one by one. ### Step-by-Step Solution: 1. **Understanding Oxidation and Reduction**: - Oxidation involves the loss of electrons or an increase in oxidation number. - Reduction involves the gain of electrons or a decrease in oxidation number. 2. **Analyzing the Statements**: - **Statement 1**: "The algebraic sum of the oxidation numbers of all atoms in an ion is zero." - This statement is incorrect. The sum of oxidation numbers in a neutral compound is zero, but for ions, it equals the charge of the ion. For example, in sulfate ion (SO₄²⁻), the sum of oxidation numbers equals -2, not zero. - **Statement 2**: "The oxidation number is an arbitrary number. It can have positive, negative, zero or fraction values." - This statement is true. Oxidation numbers can indeed be positive, negative, zero, or even fractional in some cases. - **Statement 3**: "When a negative ion changes to neutral species, the process is oxidation." - This statement is true. When a negative ion (e.g., B²⁻) loses electrons to become neutral (oxidation number increases from -2 to 0), it is classified as oxidation. - **Statement 4**: "The oxidation number of phosphorus can vary from -3 to +5." - This statement is true. Phosphorus can exhibit oxidation states ranging from -3 (as in PH₃) to +5 (as in PCl₅). 3. **Conclusion**: - The only incorrect statement among the four provided is **Statement 1**. ### Final Answer: The wrong statement is: "The algebraic sum of the oxidation numbers of all atoms in an ion is zero."
To determine which statement is wrong regarding oxidation, reduction, and disproportionation reactions, we will analyze each statement one by one. ### Step-by-Step Solution: 1. **Understanding Oxidation and Reduction**: - Oxidation involves the loss of electrons or an increase in oxidation number. - Reduction involves the gain of electrons or a decrease in oxidation number. ...
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Oxidation reaction involves loss of electrons, and reduction reaction involves gain of electrons. The reaction in which a species disproportinates into two oxidation states ( lower and higher) is called disproportionation reaction. Which of the following statements is correct?

Oxidation reaction involves loss of electrons, and reduction reaction involves gain of electrons. The reaction in which a species disproportinates into two oxidation states ( lower and higher) is called disproportionation reaction. Which of the following is not a dispropotional reaction?

Knowledge Check

  • Which of the following is a disproportionation reaction?

    A
    `Cl_(2(g))+2OH_((aq))^(-)rarrClO_((aq))^(-)+Cl_((aq))^(-)+H_(2)O_((l))`
    B
    `Cl_(2(g))+2I_((aq))^(-)rarr 2Cl_((aq))^(-)+I_(2(s))`
    C
    `2Fe_((s))+3H_(2)O_((l))overset(Delta)rarr Fe_(2)O_(3(s))+3H_(2(g))`
    D
    `2H_(2)O_((l))+2F_(2(g))rarr 4HF_((aq))+O_(2(g))`

  • Which of the following is not a disproportionation reaction ?

    A
    `P_(4)(s)+3OH^(-)(aq)+3H_(2)O(l)toPH_(3)(g)+3H_(2)PO_(2)^(-)(aq)`
    B
    `2F_(2)(g)+2OH^(-)(aq)to2F^(-)(aq)+OF_(2)(g)+H_(2)O(l)`
    C
    `Cl_(2)(g)+2OH^(-)(aq)toClO^(-)(aq)+Cl^(-)(aq)+H_(2)O(l)`
    D
    `2H_(2)O_(2)(aq)to2H_(2)O(l)+O_(2)(g)`

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